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Chp 4 definitions

Chemistry Leaving cert Chapter 4 definitions only

QuestionAnswer
Element A substance that cannot be split into simpler substances by chemical means.
Triad and Who came up with the idea of them? Triad: group of threes elements with similar chemical properties in which the atomic weight (relative atomic mass) of the middle element is approx equal to the average of the other two. Johann Doberiner came up with the idea of Triads.
Newland's Octaves and Who came up with the idea of them? Octaves: arrangements of elements in which the first and eighth element, counting from a particular element, have similar properties. John Newlands
Mendeleev's Periodic Law When elements are arranged in order of increasing atomic weight (relative atomic mass), the properties of the elements recur periodically.
Atomic number Number of protons in the nucleus of the atom
Modern Periodic Table The modern periodic table of elements is arranged in order of increasing atomic number.
Modern Periodic Law When elements are arranged in order of increasing Atomic Number, the properties of the elements recur periodically
Mass Number Is the Sum of the number of protons and neutrons in the nucleus of an atom of that element.
Isotopes Atoms of the same elements which have different mass numbers due to the different of neutrons in the nucleus.
Relative Atomic Mass Defined as - The average of the mass number of the isotopes of the element - as they occur naturally - Taking their abundance into account - expressed on a scale in which the atoms of the carbon-12 isotopes have a mass of exactly 12 units.
Principles of mass spectrometry Is that charged particles moving in a magnetic field are deflected to different extents according to their masses and are thus separated according to these masses.
Electron Configuration Shows the arrangement of electrons in an atom of an element.
Aufbau Principle When building up an electron configuration of an atom in its ground state, the electrons should occupy the lowest available energy levels.
Hund's rule of maximum multiplicity States that when two or more orbitals of equal energy are available, the electrons occupy them singly before filling them in pairs.
Pauli exclusion principle States no more than two electrons may occupy and orbital and they must have opposite spin.
Created by: AW117
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